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In the dissociation of $PC{I}_5$ as
$PC{I}_5\left(g\right)$ $PC{I}_3\left(g\right) + C{l}_2\left(g\right)$ if the degree of the dissociation is $\alpha$ at equilibrium pressure P, then the equilibrium constant for the reaction
(1) $K_p = \frac{{\alpha }^2}{1 + {\alpha }^{2}P}$
(2) $K_p=\frac{{\alpha }^2{P}^2}{1-{\alpha }^2}$
(3) $K_p = \frac{\alpha P^2}{1-{\alpha }^2}$
(4) $K_{p }= \frac{{\alpha }^{2}P}{1- {\alpha }^2}$

The equilibrium constant for the reaction 
$N{H}_{4}N{O}_2\left(s\right)$$N_2\left(g\right) + 2H_{2}O\left(g\right)$ is given by
(1) $\frac{\left[N_2\right]\left[H_{2}O\right]}{\left[N{H}_{4}N{O}_2\right]}$
(2) $\left[{\mathrm{N}}_2\right]{\left[{\mathrm{H}}_2\mathrm{O}\right]}^2$
(3) $\frac{\left[H_{2}O\right]}{\left[N{H}_{4}N{O}_2\right]}$
(4) $\frac{\left[N_2\right]}{\left[N{H}_{4}N{O}_2\right]}$
 

In which of the reactions the equilibrium constant will have no units of concentrartion?
(1) NO(g) $\frac{1}{2}{N}_2\left(g\right) + \frac{1}{2}{O}_2\left(g\right)$
(2) $H_2\left(g\right) + I_2\left(g\right)$   2HI(g)
(3) CO(g) + $H_{2}O$(g)  $C{O}_2\left(g\right) + H_{2 }\left(g\right)$
(4) In all the above reactions

The equilibrium constant for a reaction A + 2B  2C is 40. The equilibrium constant for reaction C  B + 1/2A is:
(1) 1/40
(2) ${(1/40)}^{1/2}$
(3) ${(1/40)}^2$
(4) 40

The equilibrium constant, K for the reaction: 
$2HI\left(g\right)$ $H_2\left(g\right) + I_2\left(g\right)$ at room temperature is 2.85 and at 698K is $1.4$ $\times {10}^{-2}$. This implies that the forward reaction is
(1) Exothermic
(2) Endothermic
(3) Neither exothermic nor endothermic
(4) Unpredictable

 
For the reaction 
2A(g) + B(g)$\iff$3C(g) +4D(g)
Two moles each of A and B were taken into a 1L flask. The following must always be true when the system attained equilibrium
(1) $\left[a\right] = \left[B\right]$
(2) [A] $<\left[B\right]$
(3) [B]= [C]
$\left[A\right]+ \left[B\right]<\left[C\right]+\left[D\right]$
 

Which of the following reactions is favoured by increased of temperature?
1. $N_2+H_2\rightleftharpoons 2N{H}_3+22.9 kcl$
2. $N_2\left(g\right) +O_2\rightleftharpoons 2NO\left(g\right) -42.9 kcl$
3. $2SO\left(g\right) + O_2\left(g\right) \rightleftharpoons 2S{O}_3\left(g\right) +45.3kcl$
4. $H_2\left(g\right) + C{l}_2\left(g\right) - 44.0kcl \rightleftharpoons 2HCl \left(g\right)$

For an hypothetical reaction of the kind 
$A{B}_2\left(g\right) +\frac{1}{2}{B}_2\left(g\right) \rightleftharpoons A{B}_3\left(g\right); ∆H=-xkJ$
More AB${}_3$ Could be produced at equilibrium by 
1. Using a catalyst 
2. Removing some of B${}_2$
3. Increasing the temperature 
4. Increasing the pressure 

Inert gas has been added to the following equilibrium system at constant volume 
$S{O}_2\left(g\right) +\frac{1}{2}{O}_2\left(g\right) \rightleftharpoons S{O}_3\left(g\right)$
To which direction will the equilibrium shift ? 
1.  Forward 
2. Backward
3. No effect 
4. Unpredictable 

One mole of N${}_2$ is mixed 3 moles of H${}_2$ in one litre container. If 50% of N${}_2$ is converted into ammonia by the reaction N${}_2$(g) + 3H₂ (g) $\rightleftharpoons$  2NH${}_3$(g), then the total number of moles of gas at the equilibrium are 
1. 1.5
2. 4.5 
3. 3.0 
4. 6.0

The decomposition of N${}_2$O${}_4$ to is carried out at 280$°$C in chloroform. When equilibrium is reached, 0.2 mol N${}_2$O${}_4$ and 2 $\times$10${}^{-3}$ mol of NO${}_2$ are present in 2L solution. The equilibrium constant for the reaction N${}_2$O${}_4$ $\rightleftharpoons$ 2NO${}_2$is 
1. 1$\times$10${}^{-2}$
2. 2$\times$10${}^{-3}$
3. 1$\times$10${}^{-5}$
4. 2$\times$10${}^{-5}$

In the following equilibirian 
I : A= 2B$\rightleftharpoons C;K_{eq}=K_1$
II : C+D $3A:K_{eq}=K_2$
III: 6B + D $\rightleftharpoons 2C;K_{eq}=K_3$
Hence, relation between $K_{1, }{K}_{2}and K_3$ will be 
1. $3K_1+ K_2=K_{3 }$
2. $K_1^3 .K_2^2= K_3$
3. $3K_1+K_2^2=K_{3 }$
4. $K_1^3.K_2=K$

For the follwing gaseous equilibria X,Y and Z at 300K 
X : 2SO${}_2$$+O_2\rightleftharpoons 2S{O}_3$
Y : $PC{I}_5\rightleftharpoons PC{I}_3+C{I}_2$
Z : 2HI $\rightleftharpoons$ H${}_2$ + I${}_2$
Ratio of K${}_p$ and K${}_c$ in the increasing order is: 
1. X=Y=Z
2. X<Y<Z
3. X<Z<Y
4. Z<Y<X

$N_2+ 3H_2\rightleftharpoons 2N{H}_3$
1 mole \(N_2\) and \(3H_2\) are at 4 atm.
Equilibrium pressure is found to be 3 atm. find the \(K_p\)
1. \(\frac{1}{0.5(1.5)^3}\) 
2. \(\frac{1}{0.5(0.5)^3}\) 
3. \(\frac{3\times3}{0.5(0.5)^3}\) 
4. None of these 

4 moles of A are mixed with 4 moles of B,
when 2 moles of C are formed at equilibrium
according to the reaction A +B $\rightleftharpoons$C+ D 
The value of the equilibrium constant is: 
1. 4
2. 1
3. 1/2
4. 1/4

Which of the following can act as Lowry-Bronsted acid as well as a base ?
1. CI${}^{-}$
2. HCO${}_3^{-}$
3. H${}_3$O+
4. SO${}_4^{2-}$

In the acid-base reaction HC1 + CH${}_3$ COOH$\rightleftharpoons$ C1${}^{-}+C{H}_{3}CO\stackrel{\oplus }{O}{H}_2$ the conjugate acid of acetic acid is 
1.  $C{H}_{3}CO\stackrel{\oplus }{O}{H}_2$
2. HC1
3. H${}_3$O${}^{+}$
4. CI${}^{-}$

In the reaction HCN + H${}_2$O $\rightleftharpoons H_3{O}^{+}+ C{N}^{-}$ the conjugate acid- base pair is 
1. HCN,H${}_3$O${}^{+}$
2. HCN,CN${}^{-}$
3. $H_{2}O, C{N}^{-}$
4. $C{N}^{-},H_3{O}^{+}$

Which of the following is a base according to the Lowry-Bronsted concept?
1. I^-
2. H₃O⁺
3. HCl
4. NH₄⁺

Which of the following is strongest conjugate base ?
1. C1O${}_4^{-}$
2. HCO${}_3^{-}$
3. F${}^{-}$
4. HSO${}_4^{-}$